Classifications

• • C—CHEMISTRY; METALLURGY
  • C07—ORGANIC CHEMISTRY
  • C07D—HETEROCYCLIC COMPOUNDS
  • C07D487/00—Heterocyclic compounds containing nitrogen atoms as the only ring hetero atoms in the condensed system, not provided for by groups C07D451/00 - C07D477/00
  • C07D487/02—Heterocyclic compounds containing nitrogen atoms as the only ring hetero atoms in the condensed system, not provided for by groups C07D451/00 - C07D477/00 in which the condensed system contains two hetero rings
  • C07D487/04—Ortho-condensed systems

Definitions

• the present invention is directed to a process for preparing heterocyclic sulfonyl chloride compounds by chloroxidation of di (heterocyclyl) disulfide compounds.
• di (heterocyclyl) disulfide compounds including those that possess sensitive substituents and/or have little solubility in aqueous acids or common organic solvents can be converted to heterocyclic sulfonyl chloride compounds in good yield by chloroxidation of the corresponding di (heterocyclyl) disulfide compound if the reaction is carried out in a medium comprising a water-immiscible organic solvent, water, and a phase transfer catalyst.
• the process of the invention includes the preparation of a chlorosulfonyl substituted aromatic heterocycle compound of Formula I :
• HET represents an optionally substituted 5- or 6-membered aromatic heterocyclic moiety
• HET is defined as for compounds of Formula I
• a medium comprising a water-immiscible organic solvent, water, and an effective amount of a phase transfer catalyst at a temperature of -20°C to 60°C.
• Tetraalkylammonium salts are often preferred phase transfer catalysts and chlorinated hydrocarbon solvents are often preferred water-immiscible organic solvents. Temperatures of about -10°C to about 30°C are typically preferred. The process is advantageously applied to the preparation of many substituted 2-chloro- sulfonyl [1, 2, 4] triazolo[l, 5-c] pyrimidine compounds .
• the process of the present invention is well suited for the preparation of a broad variety of chlorosulfonyl substituted aromatic heterocycle compounds of Formula I. It is especially useful for the preparation of such compounds when the di (aromatic heterocyclyl) - disulfide compound of Formula II starting material is relatively insoluble in common water-immiscible organic solvents that are suitable for use in chloroxidation reaction media and in aqueous hydrochloric acid.
• Compounds of Formula II that are relatively insoluble include those that are less than 5 percent soluble in aliphatic chlorinated hydrocarbon solvents or aqueous hydrochloric acid at temperatures below 30°C.
• the process is more especially useful when the solubility of the di (aromatic heterocyclyl) disulfide compound of Formula II in the reaction medium is less than 1 percent at temperatures below 30°C.
• the process is also especially useful for the preparation of compounds of
• Such sensitive compounds include compounds of Formula I having substituents that react readily with hydrogen chloride or chlorine .
• Suitable heterocyclic moieties encompassed by the term HET of Formulas I and II are inclusive of 5- and 6-membered aromatic heterocyclic moieties, including 5- and 6-membered aromatic heterocyclic moieties that are fused to benzene (benzoheterocyclic moieties) or fused to 5- and 6-membered aromatic heterocyclic compounds (heterocycloheterocyclic moieties).
• Oxygen, sulfur, and nitrogen heteroatoms may be present in the heterocyclic moieties, HET.
• each single ring heterocyclic and benzoheterocyclic 5- or 6-membered aromatic moiety HET may possess one oxygen or one sulfur atom and up to three nitrogen atoms and each heterocycloheterocyclic 5- or 6-membered aromatic moiety HET (HET consists of two fused heterocyclic rings) may possess a total of up to two atoms selected from oxygen and sulfur and up to six nitrogen atoms.
• the process can be applied to prepare a wide variety of chlorosulfonyl substituted oxazoles, isoxazoles, thiazoles, isothiazoles, pyrazoles, imidazoles, 1, 3, 4-oxadiazoles, 1, 3, 4-thiadiazoles, 1, 2 , 3-thiadiazoles, 1, 2, 4-thiadiazoles, 1, 2 , 4-triazoles, benzothiazoles, indazoles, pyridines, pyrimidines, pyridazines, 1, 2 , 4-triazolopyrimidines (e.g., [l,2,4]tri- azolo [ 1, 5-a] pyrimidines & [1, 2, 4 ] triazolo [1, 5-c] - pyrimidines), 1, 2 , 4-triazolopyridazines, 1, 2 , 4-triazolo- pyridines (e.g., [1, 2, 4 ] triazolo [ 1, 5-a] pyridines)
• aromatic heterocyclic moieties HET are optionally substituted with a wide variety of typical substituents.
• substituents that are tolerated include, for example, fluoro, chloro, bromo, iodo, lower alkyl (such as methyl, ethyl, pentyl, and 1, 1-dimethylethyl) , halogenated lower alkyl (such as fluoromethyl, trifluoro- methyl, dichloromethyl, 2 , 2 , 2-trifluoroethyl, and
• the process is especially useful for the preparation of many optionally substituted chloro- sulfonyltriazolopyrimidine compounds and the preparation of 2-chlorosulfonyl[l,2,4]triazolo[l,5-c] pyrimidine compounds from 2, 2 ' -dithiobis ( [1, 2 , ] triazolo [ 1, 5-c] - pyrimidine) compounds that are relatively insoluble in chlorinated hydrocarbon solvents and in aqueous hydrochloric acid is a preferred application.
• chlorosulfonyl substituted aromatic heterocycle compounds of Formula I produced by the process of the present invention are intermediates useful for the preparation of a variety of commercial and developmental pharmaceutical and agricultural products. They are typically condensed with aliphatic or aromatic amines to produce biologically active heterocyclic sulfonamide compounds .
• phase transfer catalysts have, surprisingly, been found to increase the rate of the chloroxidation reaction involved in the process and to improve the yield of the chlorosulfonyl substituted aromatic heterocycle compounds of Formula I produced.
• the increase in reaction rate that is observed allows the process to be carried out at a lower temperature and/or in a shorter period of time than previously known processes.
• Phase transfer catalysts of all types have been found to be useful in the process.
• Phase transfer catalysts that increase the solubility of chloride ion in the organic phase of the reaction medium are believed to be the most effective.
• Such phase transfer catalysts are sometimes referred to as chloride ion transfer agents.
• Suitable phase transfer catalysts include tetrahydrocarbylammonium salts, such as tetraethylammonium bromide, tetrapropyl- ammonium chloride, tetrabutylammonium bisulfate, tetra- hexylammonium chloride, phenyltrimethylammonium chloride, methyltripropylammonium bromide, benzyltriethylammonium chloride, tricaprylmethylammonium chloride, and methyltrioctylammonium bromide .
• tetrahydrocarbylammonium salts such as tetraethylammonium bromide, tetrapropyl- ammonium chloride, tetrabutylammonium bisulfate, tetra- hexylammonium chloride, phenyltrimethylammonium chloride, methyltripropylammonium bromide,
• trihydrocarbylamine compounds behave in the same manner as tetrahydrocarbyl- ammonium salts when they are in acidic media; that is, they are often effective phase transfer catalysts performing as chloride ion transfer agents.
• the medium of the process of the present invention may initially be acidic and, in any event, becomes strongly acidic as soon as the reaction proceeds .
• Trihydrocarbylamine compounds have been found to be effective phase transfer catalysts for the process. Tributylamine and trioctylamine, for example, are useful.
• Tetrahydrocarbylphosphonium salts such as tetraphenylphosphonium chloride and tetrabutyl- phosphonium bromide
• crown ethers such as dicyclo- hexano-18-crown-6, used with or without added inorganic salts, are also suitable phase transfer agents.
• Tetrahydrocarbylammonium salts are typically preferred phase transfer catalysts and tetraalkylammonium salts (wherein benzyl is viewed as methyl substituted with phenyl and is an alkyl moiety) are generally more preferred because of their effectiveness, relatively low cost, and ease of removal from the reaction product. Tetraalkylammonium salt phase transfer catalysts having 8 to 34 total carbon atoms typically produce excellent results and those having 10 to 28 total carbon atoms are generally preferred. The anion of the tetrahydrocarbylammonium salt catalyst does not appear to be an important factor. The presence of large amounts of hydrochloric acid in the medium (formed during the reaction) results in chloride ion being the principal anion in the medium.
• Chloride, bromide, iodide, sulfate, bisulfate, nitrate, phosphate, and other common anions are suitable.
• Halide ions are generally preferred and chloride ion is typically more preferred.
• Tetrapropylammonium, tetra- butylammonium, tetrahexylammonium, tricapryl- methylammonium and methyltributylammonium halides are representative of the preferred catalysts. Under some circumstances, methyltributylammonium chloride is a specifically preferred catalyst.
• phase transfer catalyst An effective amount of the phase transfer catalyst is employed in the process. Amounts in the range of 0.001 to 0.20 moles of catalyst per mole of di (heterocyclyl) disulfide compound of Formula II are typical and it is often preferred to employ 0.002 to 0.05 moles. It is generally preferred from economic and waste control points of view to use as little catalyst as is necessary to achieve reasonably fast reaction rates and good yields .
• Water-immiscible organic solvents that are unreactive under the reaction conditions of the process and in which the chlorosulfonyl substituted aromatic heterocycle compound of Formula I being produced is at least partially soluble are employed in the reaction medium.
• Chlorinated hydrocarbon solvents such as dichloromethane, chloroform, tetrachloromethane, 1, 2-dichloroethane, 1 , 1-dichloroethane, 1, 1, 1-trichloro- ethane, trichloroethylene, tetrachloroethylene, chloro- benzene, and 1, 2-dichlorobenzene are usually preferred.
• Aliphatic chlorinated hydrocarbon solvents are typically more preferred.
• Dichloromethane is often the solvent of choice. It is usually advantageous to use a sufficient amount of the water-immiscible organic solvent to maintain the compound of Formula I being produced in solution at the conclusion of the reaction.
• Water is a required element of the reaction medium.
• the water can be added totally or in part as a diluent in the di (heterocyclyl) disulfide of Formula II starting material or as aqueous hydrochloric acid. It is often advantageous to add some of the water in one or both of these ways .
• the chloroxidation reaction produces hydrogen chloride and, therefore, the aqueous phase of the medium is acidic immediately upon initiation of the chemical reaction.
• the starting material of Formula II used possesses an acid sensitive substituent, such as a methoxy group, it is often deleterious to allow the concentration of hydrogen chloride in the aqueous phase of the medium to rise above 12 molar.
• the amounts of water and hydrochloric acid employed in the medium of the process can easily be adjusted to arrive at a suitable final concentration of hydrochloric acid in the aqueous phase.
• the amount of water employed is usually 0.1 to 1 times the amount of water-immiscible organic solvent employed. It is generally preferred to use 0.2 to 0.5 times as much. Sufficient total reaction medium is used to create a fluid reaction mixture and to promote good mixing.
• Chlorine is generally added to the reaction medium as a gas. It is typically added below the surface of the reaction medium and at as rapid a rate as possible while maintaining a relatively even distribution of the chlorine in the medium and maintaining the desired reaction temperature.
• the stoichiometry of the chloroxidation reaction requires five moles of chlorine per mole of di (heterocyclyl) disulfide of Formula II. At least five moles are generally used. It is usually preferred to use a small excess of chlorine.
• the reaction is carried out at a temperature at high enough that the chemical reaction of the process proceeds relatively rapidly and low enough that side reactions are minimized. Temperatures of -20°C to 60°C are suitable; temperatures of -10°C to 30° are generally preferred.
• the reaction is exothermic and efficient cooling is generally required.
• the reaction of the process takes place quickly and is generally complete within 10 hours. The amount of time required is dependent on a variety of factors including the chemical and physical properties of the di (heterocyclyl) disulfide compound of Formula II, the temperature, the rate of chlorine addition, the organic solvent identity and amount, the amount of water, the catalyst identity and amount, the reactor geometry, and other factors known to those in the art.
• the reaction is essentially complete when the three-phase system (two liquid phases and a solid phase) becomes a two liquid phase system. It is generally preferred to carry out the reaction under conditions wherein the reaction takes place relatively rapidly and to recover the product chlorosulfonyl substituted aromatic heterocycle compound of Formula I from the reaction medium relatively rapidly in order to avoid product decomp- osition. Sodium or potassium bisulfite or sulfite is often added to the system immediately after the reaction is complete to destroy any unreacted chlorine present.
• the chlorosulfonyl substituted heterocyle compounds of Formula I obtained as products in the process of the invention are generally recovered by first removing the aqueous phase of the reaction medium from the organic phase and retaining the organic phase. They can be used as a chemical intermediates in this form without further recovery or can be further recovered from the organic phase by conventional means.
• the compounds of Formula I prepared can be further recovered, for example, by removing the solvent and any other volatile components of the organic phase by evaporation or by distillation. They can be purified, if desired, by conventional means, such as by extraction with water or with organic solvents in which they are not appreciably soluble, by recrystallization from organic solvents, or by chromatography .
• Compounds of Formula I are generally obtained in about 85 to 96 percent of the theoretical yield in the process.
• Chlorine gas (24.5 g, 370 mmol) was added over a 5-hour period with stirring and cooling at ⁇ which time the solids present completely dissolved and the solution became greenish yellow.
• the organic phase was concentrated by evaporation under reduced pressure ending at 55°C under 40 millimeters Hg (5.3 kiloPascals) pressure to obtain 28.3 g (94.4 percent of theory) of the title compound as a 92.5 percent purity white solid.
• the compound obtained was shown to be the same as that disclosed in U.S. Patent 5,488,109.

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• 1998
  • 1998-06-25 WO PCT/US1998/013186 patent/WO1999000392A1/en not_active Application Discontinuation
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